science 10 review part 1: chemical compounds. ionic compounds

Science 10 Review

Part 1: Chemical Compounds

Ionic Compounds

Ionic Compounds

• Metal and non-metal combination

Ionic Compounds

• Metal and non-metal combination• Contains charged ions (atoms or

group of atoms that have lost or gained electrons)e.g O2-, PO4

3-

K+ , NH4+

Ionic Compounds• Metal and non-metal combination• Contains charged ions (atoms or

group of atoms that have lost or gained electrons)e.g O2-, PO4

3-

K+ , NH4+

• Ionic bond forms as a result of electron transfer.

• Ionic bond is a force of attraction between positive and negative ions


Cu2+ O2-


• E.g. CuO, NaHC2O4

Cu2+ O2-



• Ionic compounds form 3D crystals that contain many ions

Cu2+ O2-



• Ionic compounds forms 3D crystals that contain many ions

• CuO, a formula unit, represents the lowest ratio of positive to negative ions

Cu2+ O2-

Molecular compounds

Molecular compounds

• Non-metal and non-metal combination

Molecular compounds


• Form molecules

Molecular compounds


• Form molecules

• Contain covalent bonds that result from electron sharing

Molecular compounds


• Form molecules

• Contain covalent bonds that result from electron sharing

• E.g. CH4, SO2

Acids, Bases and Salts


• Acids are molecular compounds that contain hydrogen atoms. They produce the H+ ion.



• E.g. HCl = hydrochloric acid H2SO4

= sulphuric acid




= sulphuric acid

• Bases contain the hydroxide ion, OH-

E.g NaOH




= sulphuric acid• Bases contain the hydroxide ion, OH-

E.g NaOH• Salts are ionic compounds that form from

reacting acids and bases. E.g. NaCl

Phase Symbols

Phase Symbols

• Are subscripts that indicate the phase of the chemical

Phase Symbols

• Are subscripts that indicate the phase of the chemicalE.g (s) solid state; Fe(s)

Phase Symbols


(l) liquid state; H2O(l)

Phase Symbols



(g) gaseous state; O2(g)

Phase Symbols



(g) gaseous state; O2(g)

(aq) means aqueous or substance is dissolved in

water; NaCl(aq)

Dissociation equations

• All ionic compounds and acids dissociate or break up into ions when dissolved in water


• All ionic compounds and acids dissociate (break up into ions) when dissolved in water

• E.g. Ca and NO2

Polyatomic ion



• E.g. Ca and NO2 Ca2+



• E.g. Ca and NO2 Ca2+ NO2-




NO2-




NO2-

Ca(NO2)2(s)




NO2-

Ca(NO2)2(s)

calcium nitrite




NO2-

Ca(NO2)2(s) Ca2+

calcium nitrite




NO2-

Ca(NO2)2(s) Ca2+ +

calcium nitrite




NO2-

Ca(NO2)2(s) Ca2+ + 2 NO2-

calcium nitrite




NO2-

Ca(NO2)2(s) Ca2+ (aq) + 2 NO2

-

calcium nitrite




NO2-

Ca(NO2)2(s) Ca2+ (aq) + 2 NO2

- (aq)

calcium nitrite


• E.g. Ga and S Ga3+ S2-


S2-


Ga3+ S2-


Ga3+ S2-

S2-


Ga3+ S2-

S2-

Ga2S3(s)


Ga3+ S2-

S2-

Ga2S3(s) 2 Ga3+ (aq)


Ga3+ S2-

S2-

Ga2S3(s) 2 Ga3+ (aq) + 3 S2-

(aq)


Ga3+ S2-

S2-

Ga2S3(s) 2 Ga3+ (aq) + 3 S2-

(aq) gallium sulphide

ending change to ide

Science 10 Review

Part 2: Balancing Equations

Study Guide p. 110

Writing and Balancing Chemical Equations

Step 1

Write chemical equation with phase symbols if not already done.

Study Guide p. 110

Writing and Balancing Chemical Equations

Step 1

Write chemical equation with phase symbols if not already done.

e.g. Al(s) + I2(g) AlI3(s)

Study Guide p. 110

Step 2

Assign every chemical species a coefficient of ONE.

Study Guide p. 110

Step 2


e.g. __Al(s) + __ I2(g) __ AlI3(s)

Study Guide p. 110

Step 2


e.g. 1 Al(s) + 1 I2(g) 1 AlI3(s)

Study Guide p. 110

Step 3

Count the number of each atom on reactant and product side of equation (multiply coefficient and subscript).

Study Guide p. 110

Step 3


Al2(SO3)3

Study Guide p. 110

Step 3


Al2(SO3)32 Aluminum

3 Sulphur

9 Oxygen

Study Guide p. 110

Step 3


Al2(SO3)3 3 Al2(SO3)32 Aluminum

3 Sulphur

9 Oxygen

Study Guide p. 110

Step 3


Al2(SO3)3 3 Al2(SO3)36 Aluminum

9 Sulphur

27 Oxygen

2 Aluminum

3 Sulphur

9 Oxygen

e.g. __Al(s) + __ I2(g) __ AlI3(s)

Study Guide p. 110

Step 4

Increase or change the coefficients to make numbers of atoms balance on both sides of equation.

3 22

Study Guide p. 110

Step 5

Always double check your answer.

Reactants

Al = 2

I = 6

Products

Al = 2

I = 6

e.g. __Al(s) + __ I2(g) __ AlI3(s)3 22

Helpful Hints:

•Balance elements in elemental form (Fe, O2, S8, P4) last.

Study Guide p. 110

Helpful Hints:


• Balance polyatomic ions (e.g. SO42-)

as a group if they don’t break apart.

Study Guide p. 110

Helpful Hints:


• Balance polyatomic ions (e.g. SO42-)

as a group if they don’t break apart.

• Balance oxygen and hydrogen last.

Study Guide p. 110

__C8H18(s) + __ O2(g) __ CO2(g) + __ H2O(g) 25 98

16 Oxygen

9 Oxygen

25 Oxygen

+

Example:

50 Oxygen

Must double all other coefficients

__C8H18(s) + __ O2(g) __ CO2(g) + __ H2O(g) 25 98

50 Oxygen

16 Carbon

36 Hydrogen

Example:

2 16 18

50 Oxygen

16 Carbon

36 Hydrogen

Science 10 Review

Part 3: Names & Formulas of Compounds

Formulas of Ionic Compounds


• Roman Numeral in name indicates ion charge



e.g mercury (II) phosphate



e.g mercury (II) phosphate Hg2+ PO4

3-




3-

Hg2+




3-

Hg2+ PO43-




3-

Hg2+ PO43-

Hg2+




3- Hg3(PO4)2

Hg2+ PO43-

Hg2+

Naming Ionic Compounds

Naming Ionic Compounds

• Must use a roman numeral to indicate the charge of metal ions with more than one possible ion charge

Naming Ionic Compounds• Must use a roman numeral to

indicate the charge of metal ions with more than one possible ion charge

e.g Cr2O3

+3 or +2



e.g Cr2O3 Cr

Cr+3 or +2



e.g Cr2O3 Cr O2-

Cr O2- O2-

+3 or +2



e.g Cr2O3 Cr3+ O2-

Cr3+ O2- O2-

+3 or +2



e.g Cr2O3 Cr3+ O2-

Cr3+ O2- O2-

+3 or +2

chromium (III) oxide

• A roman numeral is not required when a metal has only one ion charge


e.g K2SO4


e.g K2SO4

+1 only


e.g K2SO4 potassium sulphate

+1 only

Formulas of Molecular Compounds


• Binary compounds use prefix system to indicate the number atoms of each element


• Binary compounds use prefix system to indicate the number atoms of each element

• The element furthest to the left or farthest down the periodic table is written first

Greek prefixes

1 – mono 6 - hexa2 – di 7 - hepta3 – tri 8 - octa4 – tetra 9 - nona5 – penta 10 - deca


sulphur dioxide


sulphur dioxide SO2


sulphur dioxide SO2

tetranitrogen nonaoxide


sulphur dioxide SO2

tetranitrogen nonaoxide N4O9


sulphur dioxide SO2


diphosphorus pentoxide


sulphur dioxide SO2


diphosphorus pentoxide P2O5

Naming Molecular Compounds


• Mono is never used for the first element



• Second element changes to –ide ending



• Second element changes to –ide ending

• Vowels (a, o) on prefix are sometimes omitted if followed by vowels (a, o)


• Mono is never used for the first element• Second element changes to –ide ending• Vowels (a, o) on prefix are sometimes

omitted if followed by vowels (a, o)

e.g. carbon monooxide carbon monoxide


SiO2


SiO2 silicon dioxide



N2S



N2S dinitrogen monosulphide




P4Cl6




P4Cl6 tetraphosphorus hexachloride

Science 10 Review

Part 4: Chem/Phys ChangeChemical Equations

Chemical & Physical Change


• Physical change: no new substance is formed



• Chemical change: new substance is formed




• Evidence for chemical change:




• Evidence for chemical change:energy changecolour changeformation of a precipitate (solid)formation of a gas

Energy Changes• Endothermic Reactions : energy

absorbede.g ice pack

• Exothermic Reactions: energy releasede.g. combustion

Chemical equations from Word Equations


• In Chemistry 11, a solution means something is dissolved in water. Therefore, the phase is aqueous.


• In Chemistry 11, a solution means something is dissolved in water. Therefore, the phase is aqueous.

• Must include phase symbols and balance the equation


• In Chemistry 11, a solution means something is dissolved in water. Therefore the phase is aqueous.

• Must include phase symbols and balance the equation

• Diatomic molecules: H2, N2, O2, F2, Cl2, Br2, I2


E.g.A solution of barium phosphate is mixed with aqueous sodium sulphate to yield solid barium sulphate and aqueous sodium phosphate.



Ba3(PO4)2(aq)



Ba3(PO4)2(aq)+ Na2SO4(aq)



Ba3(PO4)2(aq)+ Na2SO4(aq) BaSO4(s)



Ba3(PO4)2(aq)+ Na2SO4(aq) BaSO4(s)+

Na3PO4(aq)



Ba3(PO4)2(aq)+ Na2SO4(aq) BaSO4(s)+

Na3PO4(aq)

33 2

science 10 review part 1: chemical compounds. ionic compounds

Documents

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nahc2o4ionic compounds